Each of the following sets of quantum numbers is supposed to specify an orbital. choose the one set of quantum numbers that does not contain an error. each of the following sets of quantum numbers is supposed to specify an orbital. choose the one set of quantum numbers that does not contain an error. n = 4, l = 4, ml =0 n = 4, l = 0, ml =+1 n = 5, l = 3, ml =-3 n = 3, l = 1, ml = +2 n = 3, l = 2, ml =-3

n = 5, l = 3, ml =-3 does not contain an error.

Explanation:

Principle Quantum Numbers : It describes the size of the orbital and the energy level. It is represented by n. Where, n = 1,2,3,4....

Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3... the orbitals are s, p, d, f...

Magnetic Quantum Number : It describes the orientation of the orbitals. It is represented as . The value of this quantum number ranges from . When l = 2, the value of will be -2, -1, 0, +1, +2.

1. For  n = 4, l = 4, ml =0

n=4 and l can have value 0 to (n-1) i.e. 0,1 , 2 and 3 only. m can have 0, -1 , +1, -2, +2, -3 and +3 values. Thus l= +4 is not correct.

2. For n = 4, l = 0, ml =+1

n = 4  and l can have value 0 to (n-1) i.e. 0 , 1, 2 and 3 only. For l= 0 , m can have value of 0 only. Thus m= +1 is not correct.

3. For n = 5, l = 3, ml =-3

n=5 and l can have value 0 to (n-1) i.e. 0 ,1, 2 , 3 and 4 only. For l= 3 m can have 0, -1 ,+1, -2, +2, -3 ,+3 values.

4. For  n = 3, l = 1, ml = +2

n=3 and l can have value 0 to (n-1) i.e. 0, 1 and 2 only. For l= 1, m can have 0, -1 ,+1 values. Thus m =+2 is not correct.

5. For  n = 3, l = 2, ml =-3

n=3 and l can have value 0 to (n-1) i.e. 0 , 1 and 2. m can have 0, -1 ,+1, -2 and +2 values. Thus m= -3 is not correct.

the answer is 303.15 or 303

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